What is the Difference Between Ideal Gas Law and Real Gas Law?

The main difference between the ideal gas law and the real gas law lies in the assumptions made about the gas particles and their behavior. Here are the key differences:

Ideal Gas Law:

• The ideal gas law is based on the kinetic-molecular theory of gases and assumes that particles have no volume and do not interact with each other except during elastic collisions.
• The ideal gas law is expressed as PV = nRT, where P is pressure, V is volume, n is the number of moles of the gas, R is the gas constant, and T is the absolute temperature.
• Ideal gases are theoretical and do not exist in real life.

Real Gas Law:

• Real gases have particles that occupy space and interact with each other.
• Real gas law takes into account the volume of individual particles and intermolecular interactions.
• Real gases deviate from the ideal gas law, especially at low temperatures and high pressures.

In summary, the ideal gas law is a simplified model that assumes gas particles have no volume and do not interact with each other, while the real gas law accounts for the volume of individual particles and intermolecular interactions. Real gases tend to deviate from the ideal gas law at low temperatures and high pressures, but they can be approximated by the ideal gas law at high temperatures and low pressures.

Comparative Table: Ideal Gas Law vs Real Gas Law

Here is a table comparing the differences between the ideal gas law and the real gas law:

While the ideal gas law is a scientific law that describes the behavior of hypothetical ideal gases, real gas laws describe the behavior of actual gases that do not conform to the ideal gas law. The properties of real gases and their deviations from ideality depend on factors such as the strength and type of intermolecular attractive forces and the temperature and pressure at which the gas is at.